Question

Assertion: Benzylamine is more basic than aniline.
Reason: $\,N{H_2}\,$​ group is electron releasing group.
A.Assertion and Reason are true and Reason is the correct explanation of Assertion
B.Assertion and Reason are true and Reason is not the correct explanation of Assertion
C.Assertion is true Reason is false
D.Assertion is false Reason is true

Answer 1

Hint:
Amines may be classified in line with the character and number of substituents on nitrogen. Aliphatic amines contain only Hydrogen and alkyl substituents. Aromatic amines have the nitrogen atom fixed to an aromatic ring. This structural difference ends up in all other differences in their properties like reactivity, acidity, and stability.

Complete step by step answer:
Aliphatic amines are stronger bases as compared to aromatic amines. This is due to the fact that in aromatic amines, the lone pair on nitrogen is involved in delocalization with aromatic nucleus. This can be called the resonance effect. Benzyl amine is an aliphatic amine and aniline is aromatic amine. In aliphatic amines, the $ - N{H_{2\,}}$ group is connected to an alkyl group which is known as an electron withdrawing group i.e , they need +I effect. Thus, the lone pair of electrons on nitrogen are easily available. In case of aromatic amines, the $\, - N{H_2}\,$ group is fixed to a $\, - {C_6}{H_5}\,$ group, which is also an electron withdrawing group. So, the provision of a lone pair of electrons on N is decreased. Therefore aliphatic amines are more basic than aromatic amines. Hence, benzylamine $\,({C_6}{H_5}C{H_2}N{H_2})\;\,$ is more basic than aniline.
Therefore, the correct option is (B).

Note:The basicity of amines depends on:
- The electronic properties of the groups attached to them. For example, alkyl groups increase the basicity, aryl groups diminish it.
-The degree of solvation of the protonated amine, which has steric hindrance by the groups on nitrogen.
Because of the electronic effects, the basicity of an amine may be expected to increase with the number of alkyl groups on the amine. Correlations are complicated because of the results of solvation which are opposite the trends for inductive effects. Solvation effects also dominate the basicity of aromatic amines (anilines). For anilines, the lone pair of electrons on nitrogen delocalised into the ring, leading to decreased basicity. Substituents on the aromatic ring, and their positions relative to the chemical group Electron withdrawing groups decrease electron density on nitrogen atom and thereby decreasing basicity.